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Solutions for Chapter 1.6: Formal Charge

Organic Chemistry, | 9th Edition | ISBN: 9780073402741 | Authors: Francis A Carey Dr., Robert M. Giuliano

Full solutions for Organic Chemistry, | 9th Edition

ISBN: 9780073402741

Organic Chemistry, | 9th Edition | ISBN: 9780073402741 | Authors: Francis A Carey Dr., Robert M. Giuliano

Solutions for Chapter 1.6: Formal Charge

Solutions for Chapter 1.6
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Organic Chemistry, was written by and is associated to the ISBN: 9780073402741. Since 3 problems in chapter 1.6: Formal Charge have been answered, more than 25686 students have viewed full step-by-step solutions from this chapter. This textbook survival guide was created for the textbook: Organic Chemistry, , edition: 9. Chapter 1.6: Formal Charge includes 3 full step-by-step solutions. This expansive textbook survival guide covers the following chapters and their solutions.

Key Chemistry Terms and definitions covered in this textbook
  • a-Carbon

    A carbon atom adjacent to a carbonyl group

  • becquerel

    The SI unit of radioactivity. It corresponds to one nuclear disintegration per second. (Section 21.4)

  • boiling-point elevation (DTb).

    The boiling point of the solution (Tb) minus the boiling point of the pure solvent (T° b). (12.6)

  • bond enthalpy.

    The enthalpy change required to break a bond in a mole of gaseous molecules. (9.10)

  • catenation.

    The ability of the atoms of an element to form bonds with one another. (22.3)

  • Chiral center

    A tetrahedral atom, most commonly carbon, that is bonded to four different groups; also called a chirality center

  • cyanohydrin

    A compound containing a cyano group and a hydroxyl group connected to the same carbon atom.

  • Dalton’s law of partial pressures

    A law stating that the total pressure of a mixture of gases is the sum of the pressures that each gas would exert if it were present alone. (Section 10.6)

  • diene

    A compound containing two carbon-carbon p bonds.

  • empirical formula

    A chemical formula that shows the kinds of atoms and their relative numbers in a substance in the smallest possible whole-number ratios. (Section 2.6)

  • face-centered lattice

    A crystal lattice in which the lattice points are located at the faces and corners of each unit cell. (Section 12.2)

  • Le Châtelier’s principle

    A principle stating that when we disturb a system at chemical equilibrium, the relative concentrations of reactants and

  • levorotatory

    A compound thatrotates plane-polarized light in a counterclockwisedirection (-).

  • Nernst equation

    An equation that relates the cell emf, E, to the standard emf, E°, and the reaction quotient, Q: E = E° - 1RT>nF2 ln Q. (Section 20.6)

  • ozone

    The name given to O3, an allotrope of oxygen. (Section 7.8)

  • parent ion

    In mass spectrometry,the ion that is generated when the compound is ionized.

  • pH

    The negative log in base 10 of the aquated hydrogen ion concentration: pH = -log3H+4. (Section 16.4)

  • Resolution

    Separation of a racemic mixture into its enantiomers; in mass spectrometry, a measure of how well a mass spectrometer separates ions of different mass.

  • trigonal planar

    A geometry adopted by an atom with a steric number of 3. All three groups lie in one plane and are separated by 120°.

  • Zaitsev’s rule

    A rule stating that the major product of a b-elimination reaction is the most stable alkene; that is, it is the alkene with the greatest number of substituents on the carboncarbon double bond

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